History of the Atom
May 06, 2015
History of the Atom
Democritus
Proposed that all matter is composed of tiny, indivisible particles called “atomos”Today, we define an atom as the smallest part of an element that retains the chemical identity of that element
Dalton’s Atomic Theory (1807)
1) Elements are made of tiny particles called atoms.
2) All atoms of a given element are identical.
3) The atoms of a given element are different from those of any other element.
Dalton’s Atomic Theory (cont.)
4) Atoms of one element can combine with atoms of other elements to form compounds. A given compound always has the same relative numbers and types of atoms.
Dalton’s Atomic Theory (cont.)
5) Atoms are indivisible in chemical processes. That is, chemical reactions do not create or destroy atoms, they simply change the way the atoms are grouped together.
Some of Dalton’s Symbols for the Elements
Sir William Crookes (1879)
Invented the cathode ray tube and investigated electrical charges in gases.
Figure 3.7: Schematic of a cathode ray tube
John Joseph (JJ) Thomson (1903)
Discovered the negatively charged particles (0
-1e)
Proposed the “plum pudding model”
Postulated the positive particles
Ernest Rutherford (1909)
Discovered the positively charged dense central portion of the atom using his “gold foil experiment”1
1p
Figure 3.5: Rutherford’s experiment
Figure 3.6: Results of foil experiment if Plum Pudding model had been correct
Figure 3.6: Actual Results.
Figure 3.9: A nuclear atom viewed in cross section
Niels Bohr (1913)
Electrons are located in specific energy levels
Electrons move in a definite orbit around the nucleus
James Chadwick (1932)
Discovered the third subatomic particle (neutron)
Neutron has no charge and a mass of ~1 amu
10
n
Figure 3.10: Two isotopes of sodium.
Mass number (A) = protons + neutronsAtomic Number (Z) = protons
AZ X
An Ion of Sodium